Determine the id is 4.76) of a solution that is 0.100 M in acetic acid and 0.150

Question

Determine the id is 4.76) of a solution that is 0.100 M in acetic acid and 0.150 M in sodium acetate (pK. of Question S the concentration of HCI? ml of a o.126 M solution of Ba(OH), is titrated with a solution of HCI of unknown molarty. equalence point of the titration is obtained after addition of 28.3 mL of HC, what is the molar (Ba(OH), + 2 Ha 2 H,o + Bach) Multiple choice questions Question 10 Indicate the salt which reacts with water (hydrolyzes) to produce a basic solution. a) NaczHj02 b) NHaCI c) NaNO d) BaSO4 Question 11 Indicate the pair which constitutes a buffer in aqueous solution. a) KCI and NaC b) NHs and NHaCI c) HBr and KB d) HNO, and NHaNO

Explanation / Answer

8)

we have below equation to be used:

This is Henderson–Hasselbalch equation

pH = pKa + log {[conjugate base]/[acid]}

pH = pKa + log {[CH3COONa]/[CH3COOH]}

= 4.76+ log {0.15/0.1}

= 4.94

Answer: 4.94

9)

we have the Balanced chemical equation as:

Ba(OH)2 + 2 HCl ---> BaCl2 + 2 H2O

Here:

M(Ba(OH)2)=0.126 M

V(Ba(OH)2)=25.0 mL

V(HCl)=28.3 mL

According to balanced reaction:

2*number of mol of Ba(OH)2 =1*number of mol of HCl

2*M(Ba(OH)2)*V(Ba(OH)2) =1*M(HCl)*V(HCl)

2*0.126*25.0 = 1*M(HCl)*28.3

M(HCl) = 0.223 M

Answer: 0.223 M

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